bond lengths

Moderators: Chem_Mod, Chem_Admin

josmit_1D
Posts: 107
Joined: Fri Aug 09, 2019 12:17 am

bond lengths

Postby josmit_1D » Tue Oct 29, 2019 11:14 am

why do single, double, and triple bonds have different lengths?

Benjamin Feng 1B
Posts: 102
Joined: Sat Sep 07, 2019 12:19 am

Re: bond lengths

Postby Benjamin Feng 1B » Tue Oct 29, 2019 11:18 am

The more electrons that interact with the bond, the stronger the attraction of the electrons to the nucleus, meaning that the 2 nuclei get pulled closer together and are shorter.

Cynthia Gong 1L
Posts: 51
Joined: Fri Aug 09, 2019 12:15 am

Re: bond lengths

Postby Cynthia Gong 1L » Tue Oct 29, 2019 12:08 pm

Double and Triple bonds have more electrons, so they exert a stronger attractive force on the nuclei of the other atom, thus pulling the two atoms close together and reducing the bond length.

Alexa Hernandez 3k
Posts: 74
Joined: Sat Sep 14, 2019 12:16 am
Been upvoted: 1 time

Re: bond lengths

Postby Alexa Hernandez 3k » Tue Oct 29, 2019 12:12 pm

The more Bonds means a stronger pull so consequently you also get a smaller length because of the increased attraction.

Mariah
Posts: 104
Joined: Fri Aug 02, 2019 12:16 am

Re: bond lengths

Postby Mariah » Tue Oct 29, 2019 1:21 pm

Alexa Hernandez 3k wrote:The more Bonds means a stronger pull so consequently you also get a smaller length because of the increased attraction.


So the smaller the bond, the stronger it is?

Cassandra_1K
Posts: 49
Joined: Wed Sep 18, 2019 12:16 am

Re: bond lengths

Postby Cassandra_1K » Thu Oct 31, 2019 9:08 pm

Can someone please explain and give an example of bond dissociation energy?

ABombino_2J
Posts: 102
Joined: Thu Jul 11, 2019 12:15 am

Re: bond lengths

Postby ABombino_2J » Fri Nov 01, 2019 12:12 pm

Bond dissociation is the energy required to break a chemical bond. For example, to break an H--H bond, the bond dissociation energy is 436D.

Junxi Feng 3B
Posts: 52
Joined: Sat Sep 14, 2019 12:17 am

Re: bond lengths

Postby Junxi Feng 3B » Fri Nov 01, 2019 12:49 pm

Obviously, they do not have the same length. Single bond has the longest bond length, and triple bond has the shortest bond length. This also has something to do with bond strength.

Rory Simpson 2F
Posts: 106
Joined: Fri Aug 09, 2019 12:17 am

Re: bond lengths

Postby Rory Simpson 2F » Fri Nov 01, 2019 1:06 pm

Mariah wrote:
Alexa Hernandez 3k wrote:The more Bonds means a stronger pull so consequently you also get a smaller length because of the increased attraction.


So the smaller the bond, the stronger it is?


A stronger bond will typically be shorter and have a larger dissociation energy because there are more electrons acting in the bond, making the attraction stronger.

Hannah Romano 4D
Posts: 55
Joined: Sat Aug 24, 2019 12:18 am

Re: bond lengths

Postby Hannah Romano 4D » Fri Nov 01, 2019 1:26 pm

single bonds are the longest. then double bonds are shorter. triple bonds are shortest. additionally, the shorter the bond the stronger it is.

Charysa Santos 4G
Posts: 107
Joined: Wed Sep 18, 2019 12:21 am

Re: bond lengths

Postby Charysa Santos 4G » Fri Nov 01, 2019 1:28 pm

The bond length is determined by how many bonded electrons there are. The more electrons are bonded (i.e. a triple bond in which 6 electrons are bonded), the shorter the bond length. That means that a triple bond has the shortest length (and has the most attraction/energy bringing the two atoms together), double bonds have the second shortest length, and single bonds have the longest lengths.


Return to “Bond Lengths & Energies”

Who is online

Users browsing this forum: No registered users and 3 guests